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unit 5 AP chem
vocabulary for unit 5
| Term | Definition |
|---|---|
| chemical kinetics | area of chemistry that concerns reaction rates |
| reaction rate | change in concentration of a reactant or product per unit of time |
| instantaneous rate | value of the rate at a particular time |
| rate law | also known as differential rate law |
| rate constant | property constant in the relationship between reaction rates and reactant concentration |
| order | positive or negative exponent determined by experiment of reactant concentration in a rate law |
| differential rate law | experiment gives rate of reaction as a function of concentration often called the rate law |
| integrated rate law | exponent that shows the concentration of a reactant as a function of time |
| method of initial rates | method for experimentally determining the form of the rate law for a reaction |
| initial rate | instantaneous rate determined just after reaction begins |
| overall reaction order | sum of n + m |
| first order reaction | rate of reaction depends on a concentration to the first power |
| integrated first order rate law | will always plot a straight line |
| half life of a reactant | time required for a reactant to reach 1/2 its original concentration |
| integrated second order rate law | rate of reaction depends on concentration to second power |
| zero order reaction | rate is always constant |
| integrated zero order rate law | plot of concentration of A versus t gives a straight line slope of -k |
| pseudo first order rate law | law obtained by simplification of a more complicated one |
| reaction mechanism | series of elementary steps involved in chemical reaction |
| intermediate | species is neither a reactant nor a product but is formed and consumed in the reaction sequence |
| elementary step | reaction whose rate law can be written from its molecularity |
| molecularity | number of species that must collide to produce the reaction represented by an elemental step in a reaction mechanism |
| unimolecular step | reaction step involving only 1 molecule |
| bimolecular step | reaction involving collision of 2 molecules |
| termolecular step | reaction involving the simultaneous collision of 3 molecules |
| rate-determining step | slowest step in a reaction mechanism, determines overall rate |
| collision model | model based on an idea that molecule must collide to react used to account for observed characteristics of reaction rates |
| activation energy | threshold energy that must be overcome to produce a chemical reaction |
| activated complex (transition state) | arrangement of atoms found at top of potential energy barrier as a reaction proceeds from reactants to products |
| molecular orientation | orientation of molecules during collision some of which can lead to reaction while others cannot |
| steric factor | factor (always less than 1) reflects fraction of collisions with orientation that can produce a chemical reaction |
| Arrhenius equation | equation representing rate constant as k=Ae ^-E/RT |
| frequency factor | A replaces zp |
| enzyme | large molecule, usually a protein that catalyzes biological reactions |
| catalyst | substance that speeds up a reaction without being consumed |
| homogeneous catalyst | present in the same phase as reacting molecules |
| heterogeneous catalyst | exists in different phases |
| adsorption | collection of 1 substance on the surface of another |
Created by:
mrsklann
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